Chapter 6 Things to Memorize • Chemical equilibrium- the state in which the concentrations of all reactants and products remain constant with time and the rates of forward and reverse reactions are equal. • Haber process : N 2(g) + 3H 2(g) ↔ 2 NH 3(g) • All K values are not corrected for the effects of non-ideality (gasses at high pressure and concentrated aqueous equilibria) • Law of mass action applies to solution and gaseous equilibria • When the balanced equation for a reaction is x*n, K eq = (K original ) n • 1 K eq , but infinite # of equilibrium positions • K p = K (RT) ∆n o ∆n is the Σ of the coefficients of the gaseous products – Σ of the coefficients of gaseous reactants • True K eq involves ratio of pressure or concentration at equilibrium for a substance to its reference pressure or concentration ratio to its activity. • Size of K eq and time required to reach equilibrium are NOT related • Write BALANCED reactions • At equilibrium: o Add an inert gas (one not involved in the reaction) at constant volume  increase in P total , but NO EFFECT on concentrations or partial pressures o Change the volume of the container

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